Objective/Warm-Up

• SWBAT review topics for the final.

• If you have 30 g of NaCl or 100 g of NaCl, which would have the greater % of Cl? Why?

• Calculate the % of Cl in 100 g of NaCl.

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Objective/Warm-Up

• SWBAT review topics for the final.

• Perform the following conversions:• 420.27 g Pb(CO3)2 = ______________ moles

• 33.2 g KCl = _____________ formula units• 7.2 x 1020 atoms Cu = _____________ grams Cu

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• Percent Composition- mass of element x100%total mass

• Empirical Formula- simplest ratio of elements• Molecular Formula- “unreduced”, real, actual

formula of elements• Examples:

Empirical Formula

CH2O NO2 HO

Molecular Formula

C6H12O6 N2O4 H2O2

Change from Empirical to Molecular

• A compound has a molecular mass of 90 g/mol and an empirical formula of HCO2, what is the molecular formula?

Percent Hydrate

• If you have a hydrate that weighs a total of 150 grams and you heat it so that only 70 grams are left, what percent was water?

C. Types of Yields of ProductsC. Types of Yields of Products

1.1. Theoretical YieldTheoretical Yieldthe calculated amount that the calculated amount that should be producedshould be produced

2.2. Actual YieldActual Yieldthe measured amount of a the measured amount of a productproduct

3.3. Percent YieldPercent Yieldthe efficiency of the reaction the efficiency of the reaction found from the ratio of the found from the ratio of the actual yield to the theoretical actual yield to the theoretical yield x 100 ( A/T x 100)yield x 100 ( A/T x 100)

1.1. When the proper amount of NHWhen the proper amount of NH33

reacts with enough Oreacts with enough O22, , 120.0 g120.0 g

of NO was produced. Tom of NO was produced. Tom performed the experiment, but performed the experiment, but actually produced actually produced 98.0 g NO98.0 g NO. . What is the % yield of NO?What is the % yield of NO?

D. % Yield Stoichiometry D. % Yield Stoichiometry ProblemsProblems

4 NH4 NH33 + 5 O + 5 O22 4 NO + 6 H 4 NO + 6 H22OO

98.0 g NO

120.0 g NO

X 100 = 81.7%

2. When 36.8 g of NH2. When 36.8 g of NH33 react with react with

excess of oxygen, the actual excess of oxygen, the actual yield of water is yield of water is 56.2 g56.2 g. What . What is the % yield of water?is the % yield of water?

36.8 g NH3

68.16 g NH3

X 108.1 g H2O =

58.4 g H2O56.2 g H2O

58.4 g H2O

X 100 = 96.2%

Warm-Up:2AlCl3 2Al + 3Cl2

If 35.0 g of aluminum chloride are decomposed, how many grams of chlorine are produced?What is the percent yield if only 8.50 g Cl2 are produced?

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YOU HAVE ONLY ONE MINUTE LEFT ON THIS QUESTION

0:590:580:570:560:550:540:530:520:510:500:490:480:470:460:450:440:430:420:410:400:390:380:370:360:350:340:330:320:310:300:290:280:270:260:250:240:230:220:210:200:190:180:170:160:150:140:130:120:110:100:090:080:070:060:050:040:030:020:010:00Objective: SWBAT use stoichiometry to solve limiting reactant problems using a balanced chemical equation.

35.0 g AlCl3X 1 mol AlCl3 133.35 g AlCl3

X 3 mol Cl2 2 mol AlCl3

X 70.9 g Cl2 1 mol Cl2

=27.9 g Cl2

% yield=8.50 g/27.9 g Cl2 x100% = 30.5%

Concentration

• Concentration- amount of solute in a given amount of solvent or solution

• Molarity- moles solute

L solution

• molality- moles solute

kg solvent

Acids and Bases

Acid Base

Arrhenius Releases H+ ions (HCl)

Releases OH- ions (NaOH)

Bronsted-Lowery

H+ (proton or hydronium ion) donor (HCl)

H+ (proton or hydronium ion) acceptor (NH3)

Lewis Electron pair acceptor (BH3)

Electron pair donor (NH3)

Types of Mixtures

• Solution- a homogeneous mixture, particles in a solution are about the size of molecules, approximately 1 nanometer

• Suspension- Those that make up suspensions are larger than 1,000 nanometers.

• Colloid- mixtures whose particles are larger than the size of a molecule but smaller than particles that can be seen with the naked eye. Finally, colloidal particles range in size between 1 and 1,000 nanometers. Colloids are also called colloidal dispersions because the particles of which they are made are dispersed, or spread out, through the mixture.